Fe2o3 (molar mass = 159.7 g/mol) reacts with co (molar mass = 28.0 g/mol) according to the equation fe2o3 (s) + 3 co (g) → 3 co2 (g) + 2 fe (s). when 352 g fe2o3 reacts with excess co, how much fe (iron) is produced? 1. 4.41 mol fe 2. 0.907 mol fe 3. 147 g fe 4. 25.1 mol fe

Question

Chemistry

Austin Spencer

27 March, 04:55

Fe2o3 (molar mass = 159.7 g/mol) reacts with co (molar mass = 28.0 g/mol) according to the equation fe2o3 (s) + 3 co (g) → 3 co2 (g) + 2 fe (s). when 352 g fe2o3 reacts with excess co, how much fe (iron) is produced? 1. 4.41 mol fe 2. 0.907 mol fe 3. 147 g fe 4. 25.1 mol fe

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Yahir Zhang · Answer 1

The balanced equation for the above reaction is as follows

Fe₂O₃ + 3CO - - - > 3CO₂ + 2Fe

Fe₂O₃ reacts with excess CO, which makes Fe₂O₃ the limiting reactant. the amount of products formed depends on the amount of limiting reactant present.

Number of moles of Fe₂O₃ reacted - 352 g / 159.7 g/mol = 2.204 mol

stoichiometry of Fe₂O₃ to Fe is 1:2

number of Fe moles formed - 2 x 2.20 mol = 4.408 mol

therefore number of Fe moles formed - 4.41 mol

answer is 1. 4.41 mol Fe